Chapter #1: Intro to Matter, Energy, & Measurement

What is chemistry?

A state of matter, it’s properties, and the change it goes through.

What are the 4 major benefits of study chemistry?

Energy, biochemistry, technology, and medicine

Matter

Anything that has mass & takes up space.

What are the different states of matter?

Solid, liquid, and gas

What are the properties of a solid state?

Has a fixed shape and volume; molecules are extremely close and have intricate structures with little to no movement; non-compressible molecules

What are the properties of a liquid state?

No fixed shape, but has a fixed volume; molecules are close together, but has lots of movement; molecules aren’t compressible

What are the properties of a gas state?

No fixed volume or shape; molecules are for apart from one another with fast movement; gas molecules are compressible when in a container.

What is the movement that occurs in solid molecules?

Solid

Substance

A distinct set of properties and composition that doesn’t change from sample to sample.

What are the 2 types of substances?

Elements and compounds

Elements

A substance that can’t be broken down into simpler substances.

Compound

A substance that can be broken down into simpler substances since it’s made of more than 1 element..

How many elements are currently known?

118

How many elements make up 90% of the human body mass?

Only 3; including oxygen

Law of constant composition or law of definite proportions

Compounds have a limited composition so the relative # of atoms of each element; a compound is the same for any sample.

Mixtures

Composed of multiple substances.

What’s the difference between a substance and a mixture?

A substance can’t change it’s composition but a mixture can

What are the 2 different types of mixtures?

Heterogenous and Homogenous

Heterogenous mixture

A sample mixture that varies in composition

Homogenous mixture

A mixture that has the same composition throughout.

If a homogenous form of matter has variable composition, is it a homogenous mixture of pure substance?

Homogenous mixture

If a homogenous mixture mixture doesn’t have variable composition?

It’s a pure substance.

If the substance is a pure and it contains more than one kind of atom, is it an element or compound?

Compound

1 kg is equal to how many pounds?

2.20 lbs

Physical Properties

Can be observed without changing a substance into another.

Chemical properties

Only observed when a substance is changed into another substance.

Intensive Property Types

Independent of the substance that is present

Extensive Property Types

Dependent on the amount of substance present.

Example of chemical properties

Flammability or the ability to burn oxygen

Example of physical property

Color, odor, or density

Example of intensive properties

Density

Example of extensive property

Mass, volume, or energy

Physical changes

When a substance moves between the 3 states of matter without changed the substance

Chemical changes

Chemical reactions that result in a new substance.

What physical properties can help signify a chemical change?

Change in color

Mass

Measurement of the amount of material in an object.

What is the bass unit of measurement in SI?

Kilograms (kg)

What is the base unit of measurement of the metric system?

Grams (g)

Length

The measurement of distance, where m is the base unit.

One m is equal to?

1.09 yds

What are the volume units?

Liters and milliliters

Length

Measure of distance in meters (base unit).

Kelvin to celcius conversion

K = C + 273.15

1 cubic cm is equal to how many mL

1 mL

Density

A physical property of a substance

Density formula

mass (m) / volume (v)

Water density formula

1g/mL

Significant figure general rules

All non zero digits are significant; zeroes between non-zero digits are significant; zeroes at the beginning of a # are never significant; zeroes at the end of a # are significant

Significant figures calculation rules

When addition or subtraction is performed, answers are rounded to the least significant decimal place; when multiplication or division occurs, they are rounded to the same # of significant digits as the measurement with the fewest sig figs; and only round at the end.

Dimensional analysis

Solving unit-driven problems